1. Unique Properties of Water
Chapter 2 Biochemistry
Unique Properties of Water

2. Life on Earth could Not exist without water.
Water is one of the most important, stable, and abundant molecules found in living things.
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3. Water’s Molecular structure
Water molecules consist of two hydrogen atoms and one oxygen atom that are held together by a covalent bond.
Covalent bonds are formed between atoms that are sharing electrons

4. Water’s Molecular structure
The atoms in a water’s covalent bond do not share the electrons equally.
The oxygen pulls on the electrons more strongly than the hydrogen atom.
This causes the water molecule to be a polar molecule.
Normal orbit if hydrogen’s electrons

5. Water’s Molecular structure
Due to electrons (which have a negative charge) spending more time near the oxygen atom, the oxygen side of the atom is considered negative.
While the hydrogen side of the water molecule gains a positive charge due to the protons (which have a positive charge)
For this reason, water is described as a polar molecule.

6. Water – the universal solvent
Table salt is an ionic compound that is needed by organisms.
Salt is an ionic compound because it contains two ions with opposite charges: NA+ (sodium ion) and cl- (Chlorine ion)

7. Water – the universal solvent
When table salt is mixed with water, the polar water molecule pulls apart the sodium and chlorine ions ~ dissolving salt.

8. Water – the universal solvent
The ability of water to dissolve ionic compounds is essential to life.
The proper concentration of ions (calcium, potassium, sodium, chloride) are essential to the functioning cells.

9. Water – the universal solvent
Water also dissolves other polar molecules such as glucose.
Because water can dissolve many substances it is known as the universal solvent.

10. Water – the universal solvent
Some substances do not dissolve well in water.
Lipids are composed of non polar molecules.
Lipids are insoluable (don’t break down) in water
Cell membranes are composed of lipids, which create a water-resistent barrier around the cell.

11. Adhesion vs. cohesion
Cohesion – water molecules creating hydrogen bonds with other water molecules.
Cohesion causes high surface tension – more force is needed to break the surface of a liquid.
Beading water is caused by cohesion.

12. Adhesion vs. cohesion
Adhesion – is the tendency of water to stick to substances other than other water molecules.
This is due to hydrogen bonds – water sticking to glass.

13. Usage of Adhesion & cohesion
Tall plants are able to move water from their roots to the upper branches without using energy.
Plants move water through interconnected, tube like cells.

14. Usage of Adhesion & cohesion
When water in the leaves of the upper part of a tree evaporates, the water below it is pulled up to take its place – using cohesion and adhesion

15. Usage of Adhesion & cohesion
The ability of a liquid to flow against gravity in a narrow space – such as a glass tube or vascular tissue in plants – is called capillary action.

16. Water and heat energy
Another unique property of water is that it has a high capacity to absorb and retain heat – known as specific heat.
Compared to other substances, water requires more heat energy for its temperature to change.
Water also releases energy slowly.

17. Water and heat energy
Benefits of water having a high specific heat capacity:
Creates more moderate environments for organisms to live in due to water absorbing and releasing heat slowly.

18. Water and heat energy Look at these numbers of snowfall! 45 in 6.8 in

19. Water and heat energy
This same property of water makes it easier for organisms to regulate their body temperatures.
Before body temperature changes, large amounts of heat must be gained or lost.
Cold-blooded animals store heat from the sun through the day to keep them warm through the night.

20. Water and heat energy
When a liquid absorbs enough heat it will evaporate – changing it into a gas.
The amount of heat that is needed for water to change into a gas – heat of vaporization – is high!
When we sweat, water on our skin absorbs heat as it evaporates – thus cooling us down.

21. Water density
Another unique property of water is that it has a greater density as a liquid than as a solid.

22. Water density
When water reaches its freezing point, the molecules arrange themselves into an unique structure, leaving space between them.
The same amount of molecules takes up more volume, making it less dense.

23. Water density
Due to ice being less dense than liquid water, it floats on the surface of lakes and rivers.
Bodies of water freeze from the top down – the less dense ice stays above the denser liquid water.
The ice then acts like insulation for the water below it – protecting aquatic organisms from freezing.